Production of alkali metals from ferrophosphorus and alkali carbonates or hydroxides



Get. 11, 1949. L. E. BOWE 294849266 PRODUCTION OF ALKALI METALS FROM FERROPHOSPHORUS AND ALKALI CARBONATES OR HYDRQXIDES Filed Feb. 25, 1946 wATER FERROPHosPHORus 1 a 2 SODA AsH MIxER' co+ co 4 OEMIsTER 21 DRY MINERAL OIL BRIQUETTING MACHINE I2 6 v 2 OAsEs +7 9 wATER VAPOR STORAGE REHEATER E r N 1+C0+CO TANK I QU 2 REACTiON -a COOLING 22 13 Nu-OIL MIXTURE 2s 28 ;----WATER QL SEPARATOR '14 R I 15 EXTRACTOR I 29 MOTHER uouo TANK OR STILL 17 VACUUM 32 TR|SOD|UM RECEIVER 18 FILTER I r PHOSPHATE 19 31 LIQUOR STORAGE 3e $34 FERRIC v VACUUM oxIOE 47 DRYER 45 RECE'VER CRYSTALLIZER STORAGE 46 39 35 4 VESSEL49 25 l, TRIsOOIuM PHOSPHATE REDUCING STORAGE RILN VESSELS 37 POWDERED IRON STORAGE vEssEI s 43 .i NVENTOR LEQN E. BOWE ATT RNEY Patented Oct. 11, 1949 UNI-TED STAT ES PATENT PRODUCTION OF ALKALI METALS? FROM FERROPHOS'PHORUS AND. ALKAL'I" CAR- BONATES R HYDROXIDES Leon E. Bowe, Anniston, Ala.,\assig nor-:toi-Mon-- santo Chemical Company,-St. Louis,-.Mo., a corporation of Delaware Application February 25, 1946, Serial No. 650,091

11 Claims.

This invention relates to a process for producing sodium, potassium, trialkali metalv phosphates, metallic :iron and=iron oxide by the-thermal reduction of thecorresponding alkali metal carbonates by means of ferrophosphorus.

The principal object of the invention is to provide a commercially practical process for making sodium and potassiumby carrying out the above reaction in adry inertatrnosphere andunder reduced pressure.

Anadd'itional objectzis to provide a process for substantially completely eliminating phosphorus from ferrophosphorusand recovering this ele- ..mentin the form of trisodium or tripotassium phosphate.

Another object is to provide a process for recoveringthe iron content of ferrophosphorus in the form of a powdered iron product which is substantially free of oxygen and/or phosphorus.

Aiurther object-is-to provide a powdered-iron product containing less than 1% by weight of oxygen and phosphorus, which is admirably suitable-for use in powder metallurgy.

A still further object .is to provide a process for producing a ferric oxide pigment from ferrophosphorus.

Other objects willbeapparent to those skilled inthe art as the descriptionproceeds.

Inthe. pastnumerous methods have been proposed for reacting alkali metal compounds with ferrophosphorusto form trialkali metal phosphatesiron oxide and metallic iron, but to my knowledgeno one has ever succeeded'inproducing metallic sodium. or potassium by this reaction.

Now I havedevelopeda commercially feasible process whereby sodium and potassium may be produced in substantially quantitative yields by thermally reducing the corresponding. carbonates by. means of 'ferrophosphorus, which process also yields trisodium or tripotassium. phosphate and ferric oxide or metallic iron powder, all of which have well established commercial utility'in the detergent, pigment and powder metallurgy fields respectively.

This process comprisesv reacting sodiumor potassium carbonate with ferrophosphorus in a dry inert atmosphere under'reduced pressure and at a temperaturewhich falls substantially within the range of from about 900C. to about 1500 0., and thereupon quickly cooling the resulting vapors to the sodium or potassium condensation temperature to separate these metals from the reaction product'. In'tl'iis process it is-essentialto use reduced pressure as-carbon monoxide'is a byproduct of-:the:reactionrand; therefore; the alkali metal 1 vapors must be rapidly vremoved from. the

reaction zone: an'diiquicklyf.'cooledsin order. to. prevent;substantial1oxidatiomofithese:metals by the abovezgas'.

(The-following equations areibelieved to represent the reactionstakingzplacez under: the above "conditions phosphorus,:butntherreactionse could have been 20 written, using-E1238, EeR and Fe5P3- equally as well. In any case, the weight ratio-oft-Nazo or .KzO tocphosphoruss isv the same whatever the phosphide usedr vIn carrying. out-the. present-invention, ferrophosphoruslcontaining 10,172;v to 30% and preferably from 2,2.% to..26l. bmweightof phosphorus, 'isgroundeto, a,.fii1ely divided state (about 200 mesh) and then intimately mixed. with water anda suitable.reactingproportion of sodium carbonateror. potassiumrcarbonate. The. resulting rmixtureuislcaked' .or. .briquetted and. charged into a, reactor. wherelthe. briquettesareidried. by heating. After .the .drying .operation,..the reactor. is evacuatedibymeanaof asuitablepump and while under a,-.vacuum..the.briquetted charge is heated to a temperature of'fromabout 900 C. .to about 1500JCI until thereaction has gone to completion. "The gaseous products thusproduced are rapidly removed from the reaction zone and quickly cooled .to separate thesodiumor potassium: therefrombycondensation. This step is preferably,carrled'out atatemperature of about 350 C: butis'atisfactory results are also obtained by. coolingflthe gaseous reaction product to. a temperature withinthe range .of'from about- 300 C. to about1700 C.

Condensation of the metallic sodium or potassium may beachievedinamr'd-esired manner, for example, by external cooling, but it*is' preferably accomplished by leadingthe gasesintoaquencher where they aresprayed with a' cooled mineral oil. In-p'lace ofmineral-oil'; any 'liquid having a relatively --lowvapor pressure -which-- difiers in specific" gravity and" does=not react with sodium may be employed.

As an alternative to the foregoing procedure, cooled non-oxidizing gases may be introduced into the gaseous reaction product in order to separate the sodium or potassium vapors by condensation. For this purpose nitrogen, hydrocarbons, hydrogen or mixtures thereof may be employed. 7

The volume of non-oxidizing gas required varies with the relative temperatures of the sodium or potassium vapors and the gas and may be readily calculated. The lower the temperature of the non-oxidizing gas the less of it will be 'required to accomplish the desired cooling effect.

Where a gas or liquid is-used-'for cooling the gaseous reaction product" in the manner described above, it should preferably have a temperature of about C. to 100 C,

At the end of the reaction, the solid reaction product is leached with oxygen-free water in the presence of nitrogen or another suitable inert gas. The leached product containing metallic iron powder and trisodium (or tripotassium) phosphate is filtered on a vacuum filter connected with a source of inert gas which passes through the filter cake instead of air. using an inert gas is to obviate oxidation of the airon powder toiron'oxide. I-l'oWevenwhere iron oxide is the desired product instead of metallic iron, the leached product may be filtered without using an inert gas. V

After filtering the extract, the filter cake consisting essentially of metallic iron .powder is washed with oxygen-free water and the resulting extract is charged into a vacuum or another suitable crystallizer where trisodium or tripotassium i phosphate is separated from its mother liquor by cooling. The-mother liquor thus obtained is used directly or, after dilution with water, to leach trisodium or tripotassium phosphate from the solid ferrophosphorus reaction product obtained in the next batch.

The wet metallic powder is dried by means of a suitable oxygen-free inert gas and then treated with areducing gas at a temperature of about 600 C. to about 1000 C. to remove oxygen and voltatile impurities from the powder. If desired, these steps may be combined in a single operation, that is, the iron powder may be treated with powdered iron product obtained by the foregoing process will have an oxygen content of from about 0.5% to about '7 .0% or more by weight and a phosphorus content of from about 0.05% to about 2.5% weight. Those products containing 1% or less of oxygen and phosphorus are highly useful in the field of powdered metallurgy,

As stated above, where ferric oxide is the de- 1 sired product,.it is not necessary to filter the iron; powder in an inert atmosphere. The iron powder, 1 after separation by filtering or another suitable .method, is subjected to hightemperature drying j with. air or oxygen to completely convert the iron into ferric oxide. 1

For a more complete understanding of the present process reference is made to the accompanying drawing which illustrates the flow sheet of the preferred embodiment of the present invention.

Finely divided ferrophosphorus, soda ash and The purpose of Depending upon the relative proportions of the reactants and also the reducing conditions, the"j is conveyed by pipe 23 into storage tank 24 from .which it may be pumped by way of pipe to .the reducing kiln 4|.

3 Q a reducing gas at a temperature suflicient to dry water in suitable proportions are charged into a mixer 4 by means of pipes l, 2 and 3 respectively. After intimate mixing, the product is transported by conveyor 5 to a briquetting machine 6 and formed into briquettes under a pressure of from 28000 to 35000 lbs. per square inch. The briquettes are conveyed by any suitable means 1 to reactor 8 where they are heated for to minutes at 320 C. to 400 C. to remove water therefrom, the resulting water vapor being discharged from the reactor by pipe 9.

Although the invention is not restricted thereto, reactor 8 is preferably a shaft kiln having a preheater section in which the briquettes are dried, a reaction section and a cooling section in which the reacted briquettes are cooled.

After the briquettes have been dried in the preheater section of reactor 8, they are fed into the reaction section where they are heated under a pressure of from 0.4 to mm. of mercury absolute and at a temperautre of about 1000" C. until the reaction has gone to completion. In general, a heating time of about an hour is sufficient to complete the reaction.

The gaseous reaction product including metallic sodium, CO and CO2 flows by way of pipe I0 into quencher H where the sodium is condensed and separated from the gases by contact with a dry mineral oil spray, the mineral oil for this purpose being supplied to the quencher by pipe l2. The sodium-mineral oil mixture discharges by way of pipe I3 into separator 14 which is of sufiishown) to the quencher while the molten sodium collects in the bottom of the separator and is "withdrawn by pipe [,6 into a sodium storage tank or still H. The sodium thus obtained is generally of good quality, but if greater purity is desired, it may be subjected to vacuum distillation, preferably at a temperautre of about 700 C. and

the resulting sodium vapors allowed to pass into receiver I9 by pip l8.

The gases leaving quencher H pass through pipe 20 into demister 2| which may be any standard unitfor separating mist from gases such as 'a packed tower, centrifugal separator, Cottrell precipitator, etc. The oily mist separated from the gases by the demister is conveyed by pipe 22 to separator l4 where the sodium content of the mist is recovered and the remainder is combined with the mineral oil and reused in quencher ll.

After removal of the mist, the gaseous mixture The solid sodium carbonate-ferrophosphorus reaction product, after being cooled in the cooling section of reactor 8, is discharged by pipe 25 into extractor 21 where it is leached by means of oxygen-free water and/or trisodium phosphate mother liquor, these materials being introduced by means of pipes 28 and 29 respectively. The

. leached product consisting essentially of metallic -iron powder and trisodium phosphate solution is then conveyed by any suitable means 30 into a vacuum filter 3| where the trisodium phosphate solution is separated from the iron powder.

The trisodium phosphate solution flows by pipe 32 into a storage tank '33 from which it is discharged by pipe 34 into crystallizer 35.

: The:trisodiuml'phosphateimother. .liquor isrconveyed by pipe 29 for reusexid-themrocess in the '.manner above described.

The metallic tiron aipowder separated "by the and then conveyed by'iany suitable .means 38 .to receiver 39. .Thepowder.thusobtained is in many instances of su'fficient purity to be suitable for use inpowder -metallurg directlm but 1 preferably subject the powder to treatment with are'ducing gas to removevolatile' impurities and oxygen.

"When the preferred procedure is-adopted, the iron powder is transportedby -conveyor40- into reducing kiln 4| which includes 'a 're'd-ucing-section and a cooling sectionw-finot shown). The metal powder is heated to a temperature within the range offrom'fioo' to 1000": Cfiandpreferably at a. temperature of1'850f".and"then' simultaneously or subsequently treated'with a'mixture of carbon dioxide and carbon monoxidawhich is conveyed by. means 'of pipeizifromstoragetank 24 into the reducing. kiln"4l. "The treatment with the above gaseous mixture .iscontinued until the metal powdershows no further loss in weight or until an analysisishows'that the product con- .tainsless than 1% by weight of oxygen.

After coolingin the reducing-kiln in the presenceof an inertatmosphera-the metal powder is discharged byway of outlet fl into storage .vessels 43.

Where iron oxide isdesired instead of metallic iron powder; thelatter mayrbe filtered or otherwise separated 'from the. trisodium phosphate :solution without lthewnecessity: of avoiding contact with oxygen. -However, in order to be of value as a pigment,wthe' iron-:powdershould be completely. oxidized-and it'is,'therefore, trans- ;ported by. conveyor 45 to ahigh temperature dryer 46. After conversion to ferric oxide, theproduct is conveyed by'any suitable means to a storage vessel 49.

The following table includes a number of typical runs which illustrate in a-general way'the efiect'of varying the .lratio :of. the reactants, the temperature of the reaction and-the time of heating.

.aported tby a-conveyorf 36 i=to trisodiumnnh s istorageivessels :31

"$6 .With .reference to "temperature '.variation,' a :comparison of runs 1, 7, and,8, .using approxiamately the same NazO/P" weight ratio, indicates that. thesodium volatilization is increased from 44%..to 84% or.90%.

In runs 3, 4, 5, and. 6, it will be noted that the sodium volatilization. varies .as follows.

'30 minutes, 65% Run 3 LS-minutes, 69% Average'of runs 4 and 5 -60 minutes, 80% Run 6 Preparation of briquettes- The reactants are finely divided and intimately mixed with a small amount of- Water in a pug mill or another-suitable mixer until. a substantially homogeneous composition is obtained. Thiscomposition is briquetted and dried to remove water which, if not eliminated, will interferewiththe production of sodium-or potassium. .'In the briquetting operation, a-pressure'of from 28000 to 35000lbs. per square inch is preferably employed, butit is to be understoodthat the invention is .not restricted thereto.

Thermal reduction of carbonates "by means of jerrophosphorus T-hereaction .between ferrophosphorus and the I carbonatesof sodiumand potassium is carried out in adry inert atmosphere under an. absolute pres- .sureof from .about.0.4--mm. toabout50 mm. of mercury andat a temperature whichialls substantially within the rangeof from=about 900 C. to about .1500. C. The most-satisfactory results, however, are obtainedat a temperature of. from 900 C. to 1000 C. and at an absolute pressure TABLE Ferrophosphorus-Soda ash reaction 1 '2 3 4 5 e 7 s 9 10 11 12 1s 14 Charge Reaction Conditions Analyses of Metal Powder 7 I Sodium Carbon- Rnn Ratio Temp k Minutes Pressure On Reduction Volatilate, Used, No. O/P 0. (mm. Hg.) with H2 ized, For Per cent Soda Ferro- 2 H2,.Loss, cent Ash, g. phos.,' g. At 900 0 Per cent P P M P er n, er Temp; to T Imtlal Fmal .cent cent.

5. 785 -4. 32 -900 3 3 3.67 2. 60 3. 76 44 79. 5 6. 502 5. 12 1, 000 30 16 3 4 0. 52 0. '4. 00 49 78. 4 6. 192 5. 47 l, 000 30 22 2 4 l. 00 0. 049 4. 00 65 84. 2 6. 491 5. 24 1', 000 29 I 2 3 5. 80 0. 15 4. 08 66 85. 5 6. 117 52 42 I, 000 45 15 2 3. 5 4. 0. 14 3. 85 72 S7. 3 5.321 5. 1,000 60 22 2 2+ 5.57 0.091 4.08 90.4 6.329 4.03 1,000 30 20 2 2+ 0.54 2.27 3.84 84 95.0 6.854 4.03 1,000 '30 25 3 3 0.89 2.21 3.69 96.8

1 Per cent of Na charged which is not converted to TSP.

Thus runs 1;8,-and 7 and runs 26"inclusive show that if the NazO/P 'weight' ratio is increased a from 4.03 to"4.*32:;to '5.12.'to 5.7, the phosphorus content is .--reducedwf-rom: 2.6%. to :-.about .01 or less.

iof fromfla'bout- 0.4 toabout 3 mm. of mercury.

Referring specifically to the preferred embodimentf of thepresent invention; that is. the thermal reduction of sodium carbonate by means'of ferro- .-.iphosphorus, the reactants are preferably -emtion temperature of these metals.

{17 ployed in a sodium carbonate/ferrophosphorus weight ratio of from 1.067 to 2.67, but higheror lower ratios may also be employed so long as'the theoretical requirementslare met. -CllSld8Iillg the proportions of reactants on the basis of- NazO/Pweight ratio and looking at the'reaction from the standpoint of producing a substantially oxygen-free iron powder, I prefer to carry out the reaction using ferrophosphorus and so'dium carbonate in a NazO/P ra'tio'of from about 5.3 to

1 sodium carbonate are preferably employed in a,

NazO/P weight ratio of about 5.7, but if an iron powder which is substantially free of both phosphorus and oxygen is desired, these reactants are used in the proportions adapted to supply a NazO/P weight ratio of from 5.12 to 5.47.

Sodium and potassium condensation step In order to prevent the sodium and potassium from being oxidized by 'the' carbon monoxide contained in the gaseous-product, the sodium and potassium vapors must be rapidly removed from the reaction zone and quickly cooled to a temperature correspondingtoor below the condensa- Hence it is essential that the reaction be carried out under reduced pressure so that the gaseous reaction products can be removed'from the reaction zone at a high velocity into a condenser where they can be rapidly cooled to the desired temperature.

Any suitable condenser may be employed for condensing the sodium and potassium so long as provision is made for preventing contact with air, oxygen or other oxidizing gases or compounds. However, I prefer to use a quencher in which a cooled mineral oil, such as kerosene, is sprayed into the gaseous reaction product to cool it to the required temperature. I may also condense the sodium or potassium from the gaseous reaction a product by injecting therein cold non-oxidizing gases such as hydrogen, nitrogen, hydrocarbon gases and mixtures thereof.

Reduction 0] iron powder 75o When this precedure is employed to further reduce the oxygen content of the iron powder, it is carried out at elevated temperatures using a rei-' ducing gas such as hydrogen, a mixture of carbon monoxide and carbon dioxide, methane, other hydrocarbon gases and mixtures of carbonaceous reducing gases or hydrogen with nitrogen or'fa'n other suitable inert gas. I

The optimum temperature for the reduction reaction varies with the reducing gas selected, but generally I employ a temperature which falls substantially within the range of from 600 C. to

A mixture of carbon monoxideand carbon dioxide is the preferred reducing gas and when it is used, the temperature of the reaction should iron powder, and, therefore-the ratio should vary inversely with the temperature.

When hydrogen is'employed as thereducing 95 8 gas, atemperature of 1000 Czanda reaction time of two hours are preferred, but these factors may fluctuate considerably without departing from the spirit of the invention.

In general, the reaction times varies with the reducing gas and also with the reaction temperature; the higher thetemperature the shorter the heating time andvice versa.

Iron powder drying step Where iron powder which is substantially free of oxygen is desired, it is essential to dry the iron powder by means of nitrogen or another suitable inert gas. This, however, is not necessary if the iron powder is to be reduced or ultimately converted into ferric oxide.

7 Extraction step Where it is desired to obtain metallic iron powder which is substantially free of oxygen without resorting to the reduction step, it is essential to use oxygenefree water and to carry out the extraction step in an inert atmosphere. However, when the reduction step is to be used or when ferric oxide isthe desired product, it is not necessary to adhere to the above conditions.

Filtering step through the filter cake instead of air.

The above precautions, however, are not necessary where the reduction step is subsequently emplayed or where ferric oxide is the desired product.

. Conve sion of iron powder to ferric oxide This step of the process merely involves drying I the'iron powder atan elevated temperature in the presence of air or oxygen and it may be carried out in any suitable manner known to the art.

Recovery of trisodinin and tripotassium phosphate from the corresponding est-tracts This operation merely consists in crystallizing the trisodium or tripotassium phosphate by cooling or vacuum evaporation and then separating the crystals by filtration, centrifuging, etc. There is nothing novel or critical about these steps and so they may be carried out in any manner known to those skilled in the art.

The foregoing description has been directed to the thermal reduction of sodium and potassium carbonate by means of ferrophosphorus, but it is to be understood that that invention is not restricted thereto as the hydroxides of sodium and potassium may also be used. The reactions which take place in the thermal reduction of the sodium and potassium hydroxide by. ferrophosphorus are believed to be represented by the following equations:

As in the case of the carbonates, the reaction atmosphere and at a temperature substantially within the range of from about 900 C. to about 1500 C. The reaction may also be executed un der reduced pressure, that is, under an absolute pressure of from about 0.4 mm. to about 50 mm. of mercury, but this is not essential to efficient operation. Contrary to the carbonate-ferrophosphorus reaction, atmospheric pressure may be employed in this embodiment of the invention since carbon monoxide is not a by-product and, therefore, it is not necessary to rapidly remove the sodium and potassium vapors from the reaction zone so that they can be quickly cooled to avoid substantial oxidation to the corresponding oxides.

In the ferrophosphorus-hydroxide reaction the sodium and potassium hydroxides melt before reaching the reaction temperature and conse quently the reactor must be equipped with a suitable agitator to insure intimate contact between the reactants. Moreover, it is essential that the reaction be carried out in a dry inert atmosphere at a temperature within the above range and that the alkali metals produced be condensed in a non-oxidizing atmosphere.

While I have described my invention in detail, it should be understood that many changes may be made without departing from the spirit thereof.

What I claim is:

1. The process which comprises reacting at a temperature of about 900 C. to about 1500 C. a compound selected from the group consisting of carbonates and hydroxides of sodium and potassium with at least the theoretical amount of ferrophosphorus required to yield the corresponding alkali metal and condensing the resulting alkali metal vapor by cooling, said reaction being carried out in a dry inert atmosphere and under an absolute pressure of from about 0.4 mm. to about 50 mm. of mercury.

2. The process defined in claim 1 wherein the reaction is carried out under an absolute pressure of from about 0.4 mm. to about 3 mm. of mercury.

3. The process defined in claim 1 wherein the reaction is carried out at a temperature of about 900 C. to about 1000 C.

4. The process defined in claim 1 wherein the reaction is carried out under an absolute pressure of from about 0.4 mm. to about 3 mm. of mercury and at a temperature of about 900 C. to about 1000 C.

5. The process which comprises reacting at a temperature of about 900 C. to about 1500 C. a briquetted mixture of sodium carbonate and ferrophosphorus in the proportions calculated to provide a NazO/P weight ratio of about 5.1 to about 5.5 and thereby producing metallic sodium, powdered iron and trisodium phosphate and.- cooling the resulting metallic sodium vapor to reaction is carried out at a temperature of about 900 C. to about 1000 C. and under an absolute pressure of from about 0.4 mm. to about 3 mm. of

. mercury.

at least the sodium condensation temperature to 8. The process which comprises reacting together at a temperature of from about 900 to about 1500 C. a briquetted mixture of sodium carbonate and ferrophosphorus in the proportions calculated to provide a NazO/P weight ratio of about 4 to about 10 and thereby producing metallic sodium and rapidly cooling the resulting gaseous product to at least the sodium condensation temperature to condense said metallic sodium, said reaction being carried out in a dry inert atmosphere and under an absolute pressure of from about 0.4 mm. to about 50 mm. of

mercury.

9. The process which comprises reacting at a temperature of about 900 C. to about 1500 C. a briquetted mixture of sodium carbonate and ferrophosphorus in the proportions calculated to provide a NazO/P weight ratio of about 4 to about 5.7 and thereby producing metallic sodium vapor, and rapidly cooling said vapor to the sodium condensation temperature to condense said metallic sodium, said reaction being carried out in a dry inert atmosphere and under an absolute pressure of from about 0.4 mm. to about 50 mm. of mercury.

10. The process which comprises reacting at a temperature of about 900 C. to about 1500 C. a briquetted mixture of sodium carbonate and ferrophosphorus in the proportions calculated to provide a NazO/P Weight ratio of about 4.0 to about 4.3 and thereby producing metallic sodium vapor, and rapidly cooling said vapor to at least the sodium condensation temperature to condense said metallic sodium, said reaction being carried out in a dry inert atmosphere and under an absolute pressure of from about 0.4 mm. to about 50 mm. of mercury.

11. The process which comprises reacting at a temperature of about 900 C. to about 1500 C. a briquetted mixture of sodium carbonate and ferrophosphorus in the proportions calculated to provide a NazO/P weight ratio of about 5.1 to 5.5 and thereby producing metallic sodium, powdered iron and trisodium phosphate and recovering at least .one of said products, said reaction being carried out in a dry inert atmosphere and under an absolute pressure of from about 0.4 mm. to about 50 mm. of mercury.

LEON E. BOWE.

REFERENCES CITED The following references are of record in the file of this patent:

UNITED STATES PATENTS Number Name Date 1,837,935 Ylla-Conte Dec. 22, 1931 1,888,003 Lindberg Nov. 15, 1932 1,939,305 Klein Dec. 12, 1933 2,391,728 McConica Dec. 25, 1945 FQREIGN PATENTS Number Country Date 338,409 Great Britain Nov. 20, 1930 

